First slide

Solubility product(KSP)

Question

Solubility of AgCl in water, 0.01 M ${CaCl}_{2},$ 0.01 M NaCl and 0.05 M ${AgNO}_{3}$ are $S_{1}, S_{2}, S_{3} and S_{4}$ respectively, then

Moderate

A

$S_{1} > S_{2} > S_{3} > S_{4}$
B

$S_{1} > S_{3} > S_{2} > S_{4}$
C

$S_{1} > S_{2} = S_{3} > S_{4}$
D

$S_{1} > S_{3} > S_{4} < S_{2}$

Solution

$AgCl ⇌ {Ag}^{+} + {Cl}^{-}$
$In {CaCl}_{2}$
${CaCl}_{2} ⇌ {Ca}^{+ 2} + 2 {Cl}^{-}$
0.01 0.01 2 x 0.01
In NaCl
$NaCl ⇌ {Na}^{+} + {Cl}^{-}$
0.01 0.01 0.01
$In {AgNO}_{3}$
${AgNO}_{3} ⇌ {Ag}^{+} + {NO}_{3} ¯$
0.05 0.05 0.05
common ion effect is maximum in ${AgNO}_{3}$
So, $S_{1} > S_{3} > S_{2} > S_{4}$

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